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CHM135H1 (333)
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Department
Chemistry
Course
CHM135H1
Professor
Kris Quinlan
Semester
Summer

Description
N.B. ^ indicates superscript LECTURE 2 Chapters 3 & 5 Slide Number Notes 23 - a mole = 6.022 x 10^23 units of something therefore sensible for calculations about atomic-scale entities - 1 mol = 12 g of ^12 C - mass to moles via dividing by gmol - moles to number of atoms via multiplying by Avogadros number - number of atoms to moles via dividing by Avogadros number - moles to mass via multiplying by gmol 24 - Ans: D - formula to determine number of molecules: 1g (1mol____g)(6.022x10^23 molecules1mol) - fill in the blank with the MWs of the four options to determine D 25 - significance of empirical formulas: when presented with unknown compound, one uses combustion analysis, which releases elemental gases present in a certain ratio (thus determining empirical formula) - EX. M is an unknown metal - Mass % = mass of element per mole of compound x 100% Mass of 1 mole of compound -
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